Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 15: Problem 31

Explain what a titration curve is, and sketch its shape.

Short Answer

Expert verified
A titration curve is a graph showing the pH of the solution versus the volume of titrant added during a titration. It has four phases: the initial phase, the buffering phase, the steep rise or fall around the equivalence point, and the final phase. To sketch it, draw a nearly flat line for the initial phase, a slightly rising or falling line for the buffering phase, a steep line at the equivalence point, and a less steep line beyond the equivalence point.

Step by step solution

01

Understand Titration Curve

A titration curve is a graph that reveals the volume of added titrant (a solution of known concentration) in relation to the pH of the solution. It's used to visualize the process of titration, which involves finding the concentration of an unknown solution (the analyte) by adding the titrant.
02

Recognize Phases of a Titration Curve

There are typically four phases in a titration curve. Before the equivalence point, when only a little titrant has been added, the curve is initially flat, representing the initial pH of the analyte. As more titrant is added, the curve rises or falls gradually. This is the buffering region, where the analyte resists changes in pH. Close to the equivalence point, the curve starts to rise or fall sharply as the titrant neutralizes the analyte. At the equivalence point, all the analyte has been neutralized by the titrant. Beyond the equivalence point, the curve starts to flatten again as the solution becomes nearly all titrant.
03

Sketch the Titration Curve

To sketch a titration curve, first draw a horizontal line for the volume of titrant and a vertical line for the pH. Start by drawing a nearly flat segment for the initial phase. Then draw a slightly rising or falling segment for the buffering region. Draw a steep slope at the equivalence point. Finally, finish with a less steep, nearly flat segment beyond the equivalence point.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Identify each of the following compounds as an acid or a base according to the Bronsted-Lowry classification. For each species, write the formula and the name of its conjugate. \begin{equation} \begin{array}{l}{\text { a. } \mathrm{CH}_{3} \mathrm{COO}^{-}} \\ {\text { b. HCN }} \\ {\text { c. HOOCCOOH }} \\ {\text { d. } C_{6} \mathrm{H}_{5} \mathrm{NH}_{3}^{+}}\end{array} \end{equation}

If the pH of a solution is \(4.3,\) what is the hydroxide ion concentration?

Group the following four terms into two pairs according to how the terms are related, and explain how they are related: end point, standard solution, titrant, and transition range.

Why are weak acids and weak bases poor electrical conductors?

A solution has a pH of \(10.1 .\) Calculate the hydronium ion concentration and the hydroxide ion concentration.
See all solutions

Recommended explanations on Chemistry Textbooks

Inorganic Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemical Analysis

Read Explanation

Kinetics

Read Explanation

Making Measurements

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free